Decomposition of CaCO3(s) into CaO(s) and CO2(g), ΔHᵒ 25ᵒ = 178 kJWrite the thermochemical equation of one mole of nitrogen gas, N2 reacts with oxygen gas, O2, two moles of nitric oxide is formed. In the process, 180.5 kJ of heat is required.Calculate the standard enthalpies of combustion at 25ᵒC of the following: ` (a) C4H8(g) + H2(g) à C4H10(g) ΔHᵒ = -2878.6kJ (b) C4H6(g) + 2H2(g) à C4H10(g) ΔHᵒ = -2543.5 kJ5 grams of an unknown compound was dissolved in 75 ml of water with an initial temperature of 22.5ᵒC contained in a coffee-cup calorimeter. Upon dissolution of the compound, the final temperature of the resulting solution is 33.2ᵒC. The calorimeter constant used is 200 J/ᵒC. What is the heat of the solution of the compound?

1. CaCO3(s) ---> CaO(s) + CO2(g) ∆H° =178KJ 2. N2(g) + O2(g) ---> 2NO(g) ∆H° = 180.5 KJ

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Decomposition of CaCO_3(s) into CaO_(s) and CO_2(g), ΔHᵒ ₂₅_ᵒ = 178 kJ
Write the thermochemical equation of one mole of nitrogen gas, N₂reacts with oxygen gas, O2, two moles of nitric oxide is formed. In the process, 180.5 kJ of heat is required.
Calculate the standard enthalpies of combustion at 25ᵒC of the following:



`         (a)      C₄H_8(g) + H_2(g) à C₄H_10(g)ΔHᵒ = -2878.6kJ

          (b)       C₄H_6(g) + 2H_2(g) à C₄H_10(g)ΔHᵒ = -2543.5 kJ
5 grams of an unknown compound was dissolved in 75 ml of water with an initial temperature of 22.5ᵒC contained in a coffee-cup calorimeter. Upon dissolution of the compound, the final temperature of the resulting solution is 33.2ᵒC. The calorimeter constant used is 200 J/ᵒC. What is the heat of the solution of the compound?

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